17. Acid and Base Equilibrium

Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The K_a value of HCN is 4.9 × 10⁻¹⁰.

An unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 

What is the pH of a 0.320 M solution of Ca(NO₂)₂ (ka of HNO₂ is 4.5 × 10^-4)?

What is the pH of a 0.750 M solution of NaCN (K_a of HCN is 4.9 × 10^-10)?

How can the pH of a solution be calculated if the pOH is known?

The K_b of methylamine is 4.4 x 10^–4. What is the approximate [OH^–] of a 1 M solution of methylamine?

calculate the pH of a 0.10 M solution of hydrazine, N₂H₄ . K_b for hydrazine is 1.3×10⁻⁶ .

What is the [OH⁻] of a 1.40 m solution of pyridine (C₅H₅N, K_b = 1.70 × 10⁻⁹)?

What is the [OH^-] of a 1.40 M solution of pyridine (C₅H₅N, K_b = 1.70 × 10^-9)?

What is the pH of a solution with a hydroxyl ion (OH^-) concentration of 10^-10 M?

The pOH of a solution is 10.75. What is the concentration of OH^– ions in the solution?

Determine the pH of a 0.227 M C₅H₅N solution at 25 °C. The K_b of C₅H₅N is 1.7 x 10^-9.

The pH of 2.65 m CH₃NH_2(aq) is 12.54. determine the value of K_b for methylamine.

An unknown weak base with a concentration of 0.170 M has a ph of 9.42. What is the K_b of this base?

What is the pH of a 0.300 M solution of aniline (C₆H₅NH₂, K_b = 4.3 × 10⁻¹⁰)?

What is the pH of a 0.300 m solution of aniline (C₆H₅NH₂, K_b = 4.3 × 10⁻¹⁰)?

What is the pH of a 0.420 M solution of C₅H₅NHBr (K_b of C₅H₅NH is 1.7 × 10^-9)?

Morphine is a weak base. a 0.150 m solution of morphine has a pH of 10.5. What is the K_b for morphine?

The pH of 2.65 M CH₃NH₂(aq) is 12.54. Determine the value of K_b for methylamine.

Determine the pH of a 0.227 M C₅H₅N solution at 25°C. The K_b of C₅H₅N is 1.7 x 10^-9.

Determine the pH of each solution. a. 0.20 M KCHO₂ b. 0.20 M CH₃NH₃I c. 0.20 M KI

Determine the pH of each two-component solution. a. 0.0550 M in HI and 0.00850 M in HF b. 0.112 M in NaCl and 0.0953 M in KF c. 0.132 M in NH₄Cl and 0.150 M HNO₃ d. 0.0887 M in sodium benzoate and 0.225 M in potassium bromide e. 0.0450 M in HCl and 0.0225 M in HNO₃

Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)₂ b. 0.265 M NH₄NO₃ and 0.102 M HCN c. 0.075 M RbOH and 0.100 M NaHCO₃ e. 0.115 M NaClO and 0.0500 M KI